If reactants are favored due to a temperature change, what is the result for Kc?

When a temperature change affects the position of equilibrium in a chemical reaction, it also impacts the equilibrium constant, Kc. If the reactants are favored as a result of the temperature change, it indicates that the equilibrium has shifted to the left, meaning that the concentration of reactants increases compared to that of the products.

Kc is defined as the ratio of the concentration of products to the concentration of reactants at equilibrium, raised to the power of their respective stoichiometric coefficients. When the concentration of reactants increases and the concentration of products decreases due to the shift favoring the formation of reactants, the numerical value of Kc decreases.

This correlation stems from Le Chatelier’s principle, which states that a system at equilibrium will adjust to counteract any changes imposed on it, including temperature changes. If the shift occurs in favor of reactants, it follows that Kc decreases accordingly. Thus, the correct result for Kc when reactants are favored due to a temperature change is a decrease.